Chemistry 30S FINAL EXAM REVIEW

Important Notes: You will be provided with: Periodic Table Ion Table Mole Road Prefixes (covalent naming) Electronegativity Table Solubility Chart Organic Prefixes Organic Suffixes Gas Laws Formulae Flow Chart for IMF’s

Unit 1 - CHEMICAL REACTIONS What you need to know: Review Concepts Determine whether a compound is ionic or covalent Determine numbers of protons, electrons, and neutrons in a compound Name ionic compounds Name covalent compounds Balancing Chemical Equations Percent Composition Determine the percent composition of any atom in a given molecule Determine the percent composition of water in a hydrate Isotopes What are they?

Calculate the average mass of an element given the percent abundance of its isotopes

Moles What is a mole? Why do we use them in chemistry? What is Molar Mass? Where do you find them? Convert between moles and numbers of molecules Convert between moles and grams Empirical and Molecular Formulas Similarities and differences between empirical and molecular formulas Determining EF based on percentages Determining MF using EF and Molar Mass Stoichiometry

Using an equation and a known amount of one substance to determine the amount of another substance

Some example questions: 1) For the atom represented by 65Zn30 determine:

a. Number of protons b. Number of electrons c. Number of neutrons d. Atomic mass (in amu)

2) Complete the following table using the correct naming system. Name Formula Ionic or Covalent?

BBr3 Iron (II) Phosphide

Disilicon Hexabromide Cr(CO3)3 PbS

Copper (I) Phosphate

3) Find the percent composition for each atom in the following:

a. Ca(OH)2 b. SF8

4) Find the percent composition of water in the hydrate CoCl2 ◦ 6 H2O. 5) What is an isotope? How do isotopes explain the non-perfect masses of the elements on the periodic table? 6) Chlorine consists of two major isotopes, one with 18 neutrons, 75.77% of chlorine atoms, and one with 20 neutrons, 24.23% of chlorine atoms. Calculate the average atomic mass of a chlorine atom.

7) What is a mole? Why is it useful in chemistry? 8) How much does one mole of Boron atoms weigh? How do you know? 9) What is Avagadro’s number? How was it chosen? 10) Calculate the number of moles in 2.06 x 1024 atoms of sodium. 11) Calculate the number of molecules of AlN3 in 0.46 moles. 12) How many moles of Barium are present in a sample having a mass of 22.3 g? 13) A chemical reaction requires 3.7 moles of Boron. What mass, in grams, of Boron must be used in the reaction? 14) A chemical reaction results in 57.2 g of CO2. How many molecules of gas were produced?

15) Calculate the mass of 0.025 moles of ammonia, NH3. 16) Calculate the number of molecules in 12.5 g of Nitrogen (N2). 17) What is empirical formula? What is molecular formula? How are they different? Are there any cases where they are the same? 18) Determine the empirical formula of a compound with the following composition by mass: 48.0 % C, 4.0 % H and 48.0 % O. 19) a) Determine the empirical formula of a compound with the following composition by mass: 60.0 % C, 12.0 % H and 28.0 % N. b) If this compound has a molar mass of 300 g/mol, what is its molecular formula?

20) Balance each of the following equations and determine whether they are synthesis, decomposition, single replacement, double replacement, or combustion reactions.

a) ___ CuSO4 + ___ NaOH ___ Cu(OH)2 + ___ Na2SO4

b) ___ OsO4 + ___ PtCl4 ___ PtO2 + ___ OsCl8

c) ___ CF4 + ___ Br2 ___ CBr4 + ___ F2

d) ___ Hg2I2 + ___ O2 ___ Hg2O + ___ I2

e) ___ Y(NO3)2 + ___ GaPO4 ___ YPO4 + ___ Ga(NO3)2

f) ___ C7H16 + ___ O2 ___ CO2 + ___ H2O

g) ___ C + ___ H2 ___ C3H8

21) Write the correctly balanced chemical equation for each of the following.

a) calcium hydroxide + carbon dioxide calcium carbonate + water

b) potassium hydroxide + carbon dioxide potassium hydrogen carbonate

c) hydrogen sulfide + lead (III) chloride hydrogen chloride + lead (III) sulfide

22) Given the unbalanced reaction Fe + S8 → FeS

a) What mass of iron is required to react with 1.8 g of Sulfur? 23) Potassium reacts with chlorine gas to produce potassium chloride. a) Write a balanced chemical equation for the reaction. b) How many grams of KCl can be produced from 5.9 g of K and excess Cl2? c) How many grams of KCl could be produced from 16.00 g of Cl2 and excess K?

Unit 2 – GAS LAWS What you need to know: Describe the basic principles of Kinetic Molecular Theory Describe the idea and conditions of STP Convert between units of pressure (mm Hg, atm, kPa) Convert between units of temperature (K and C) What is a manometer? What does it measure? Solve problems involving missing measurements on manometers

Boyle’s Law: Describe the relationship between pressure and volume and use it to solve problems (P1V1 = P2V2) Charles’ Law: Describe the relationship between temperature and volume and use it to solve problems V1 = V2

T1 T2 Gay-Lussac’s Law: Describe the relationship between temperature and pressure and use it to solve problems P1 = P2

T1 T2

Use the combined gas law to solve problems P1V1 = P2V2 T1 T2 Some example questions:

1) Determine the missing value for each of the following:

Ans. (A) = __________ Ans. (B) = __________ Ans (C) = __________

251.8 kPa 844 mm Hg

X mm Hg

1.51 atm 324 mm Hg

X kPa

95 mm Hg

105.9 kPa

X atm

2) Assuming only the parameters given change, what happens to:

a. Temperature, if the volume of a gas increases?

b. Volume, if the pressure of a gas decreases?

c. Pressure, if the temperature of the gas decreases?

3) Convert the following temperatures to Kelvin. a. 23°C b. -42°C c. 120°C

4) Convert the following pressures to the unit indicated. a. 1.75 atm to mm Hg

b. 720 mm Hg to kPa

c. 156 kPa to atm

5) What is STP? What does it stand for, what is it used for, and what are the

values associated with it?

6) If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?

7) If 10.0 liters of oxygen at STP are heated to 512 °C, what will be the new volume of gas if the pressure is also increased to 1520.0 mm of mercury?

8) The pressure of a gas is reduced from 1200.0 mm Hg to 850.0 mm Hg as the volume of its container is increased by moving a piston from 85.0 mL to 350.0 mL. What would the final temperature be if the original temperature was 90.0 °C?

9) If 15.0 liters of neon at 25.0 °C is allowed to expand to 45.0 liters, what must the new temperature be to maintain constant pressure?

10) A 40.0 L tank of ammonia has a pressure of 12.7 kPa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kPa while its temperature remains constant.

Unit 3 – SOLUTIONS

What you need to know: Saturated, Unsaturated & Supersaturated solutions: what they mean, similarities, differences, how to make them

Heterogeneous and homogeneous solutions – define and determine Solute, Solvent, Solution – define and determine Read a solubility curve and use it to answer questions What is Molarity?

Use the molarity formula (c = n/V or Molarity = mol/L) to calculate the concentration of a solution Percent volume by volume and Percent mass by mass calculations Give detailed instructions on how to make a solution Give detailed instructions (and show calculations) on how to dilute a solution Use a solubility chart to determine whether a given compound will dissolve in water or not Use the notations (aq) or (s) in a chemical equation to show whether a compound will dissolve or not Write Dissolving Ionic Equations, Overall Ionic Equations, and Net Ionic Equations for a chemical reaction Use Stoichiometry (the ratio between compounds in a balanced equation) to determine how much of a product can be formed Identify a limiting factor and use it to determine how much of a product can be formed Calculate the concentrations of remaining ions in solutions after a reaction is complete

Some example questions:

1) Describe the differences between unsaturated, saturated, and supersaturated solutions.

2) What is solubility? How do we indicate in a chemical equation whether or not a substance is soluble?

3) How many grams of ammonium sulfate are required to make 5 L of a 0.5 M solution?

4) What is the concentration of a solution of a solution with a volume of 2.5 L and that contains 6.54 g of calcium phosphate?

5) Explain how you would make the following solutions. Include directions as to how to do it. a) 250 mL of 2 M lithium nitrate b) 2.5 L of 0.75 M NaCl

6) If I dilute 250 mL of 0.5 M hydrochloric acid to a final volume of 2 L, what is the concentration of the solution?

7) If I had 5 mL of 12 M sulfuric acid and I added 105 mL of water to the solution, what would be the final concentration of the acid?

8) Which of the following solutions would generate an insoluble precipitate when combined with a solution of calcium chromate?

Ammonium hydroxide Potassium iodide Sodium carbonate

Use the solubility curve to answer the questions below. Be sure to include units!

9)a. What is the solubility of KNO3 at 10C?

____________ b. What is the solubility of KCl at 70C?

c. What is the solubility of KClO3 at

80C? ___________ d. What is the solubility of Ce2(SO4)3 at

50C? ____________

10) At 40C, you dissolved 10 g of Ce2(SO4)3 in 100 g of water. Is this solution saturated or

unsaturated?

b. How do you know?

11) a) Which compound is most soluble at 40 ºC? ________ (1)

b) Which is the least soluble at 80 ºC? ________ (1)

12) 200 mL of 0.2 M sodium sulfate solution is combined with 700 mL of 0.10

M of silver nitrate. a. What is the limiting factor in this reaction? b. calculate the mass of precipitate. c. Write DIE’s, the OIE, and the NIE (ICE table) d. Calculate the concentration of all ions in solution

Unit 4 – PHYSICAL PROPERTIES What you need to know: How to draw Lewis structures for compounds What does polarity mean? What does electronegativity mean?

Determine whether or not a bond is polar and indicate using arrows or δ notation Determine whether or not a compound is polar based on its bond polarity and shape Determine which types of Intermolecular Forces are present in a substance (Dispersion, Dipole-dipole, Hydrogen Bonding, Ion-Ion) given the IMF Flow chart Determine which compound will have the higher melting/boiling point, volatility, and vapor pressure based on IMF’s Determine whether a reaction is endothermic or exothermic Analyze a heating or cooling curve to determine melting and boiling points Analyze a phase diagram (include critical point, triple point, normal melting and boiling points) Analyze a vapor pressure diagram and relate to IMF’s

Some example questions:

1) Draw Lewis structures for the following compounds: a) CCl4 b) H2S c) CO2

2) Identify the main type of intermolecular force in each compound. a) Na2O b) Carbon disulfide

c) Ammonia (NH3) d) Oxygen e) CH2F2 f) C2H6

3) Rank the following compounds by increasing melting point. a) C2H6, C2H5OH, C2H5F

b) H2S, H2O, H2

c) BBr3, BI3, BCl3

4) Explain how dipole-dipole forces cause molecules to be attracted to each other (a diagram may help).

5) Rank the following compounds from lowest to highest boiling point: calcium carbonate, methane, methanol, dimethyl ether (CH3OCH3).

6) State whether the following processes are endothermic or exothermic: a. Snow melting b. A box exploding c. Cooking an egg

Heating Curve Name__________________ Homework Date____________Per____

ANSWER THE FOLLOWING USING THE ABOVE HEATING CURVE

1. What is the melting temperature of the above substance? _____

2. What is the freezing temperature of the above substance? _____

3. What is the boiling temperature of the above substance? _____

4. The part of the graph labeled “e” represents temperatures at which gas is being heated. Describe what is happening for each of the other lettered sections of the graph:

a. ___________________________________________________________

b. ___________________________________________________________

c. ___________________________________________________________

d. ___________________________________________________________

5. In which section of the graph are atoms moving the least? ___________

6. In which section of the graph is this substance all liquid? ____________

7. On your graph, draw an arrow to and label each of the following: “melting

begins”, “melting complete”, and “boiling begins”.

For each of questions (7) - (12), refer to the phase diagram for mysterious compound X.

(7) What is the critical temperature of compound X?

(8) If you were to have a bottle containing compound X in your closet, what phase would it most likely be in?

(9) At what temperature and pressure will all three phases coexist?

(10) If I have a bottle of compound X at a pressure of 45 atm and temperature of 1000 C, what will happen if I raise the temperature to 4000 C?

(11) Why can’t compound X be boiled at a temperature of 2000 C?

(12) If I wanted to, could I drink compound X?

Unit 5 – ORGANIC CHEMISTRY

What you need to know: Identify whether a substance is organic or not by formula Naming alkanes, including branches Naming alkenes and alkynes, including branches

General form of an alkane, alkene, and alkyne Identify an alcohol and name it Understand one method of creating an alcohol from an alkene Identify a carboxylic acid and name it Identify an ester and name it

Understand one method of creating an alcohol from a carboxylic acid and an alcohol

Some example questions:

1) Identify the following as either alkane, alkene, alkyne, alcohol, carboxylic acid, or ester.

a. CH3CH2COOH b. CH4 c. CH3CH2OH

d. C5H10 e. C7H12 f. CH3CH2COOCH2CH2CH3

2) Name the following.

a.

b.

c.

d.

e.

f.

g.

h.

i.

3) Draw the following. a. 2 – butanol b. pentanoic acid

b. 3-ethyl-2,2-dimethyl heptane d. ethyl butanoate

c. cis-4-methyl-2-hexene e. 4,5–dimethyl-2-pentyne

4) Under what conditions are the prefixes cis- and trans- required in naming an organic compound?

5) Draw and name all three isomers of pentane (C5H12)

6) Draw and name at least three isomers of hexene (C6H12). Include at least one branched isomer.

7) 2-pentene and water react at a really high temperature with an acid

catalyst.

a. What is a catalyst?

b. Draw and name the products of the reaction.

8) What is the general form of an alkane? Alkene? Alkyne?

9) Draw and name two organic compounds that would react to produce ethyl hexanoate. What is the other product of the reaction?

10) Draw and name the products of the reaction between 1-propanol and ethanoic acid.